Part C What is the pH after the addition of 25.0 mL of 0.145 M NaOH to 25.0 mL of 0.125 M HNO3? • View Available Hint(s) O 2.00 O 13.70 O 12.00 O 7.00 Submit

Q: A liter of 0.200M aquas solution of the triprote acid H3PO4 is being titrated with 1.00M aquas…

A: H3PO4 is a triprotic acid and hence undergoes dissociation in three steps. The pH of the solution is…

Q: 7-Consider the titrations of the pairs of aqueous acids and bases listed on the left. For which pair…

A: 7. Depending upon strengths of acids and bases -  the pH of the equivalent point can be determined.

Q: Calculate the percent ionization for bromic acid in a solution that contains 0.00850 M acetic acid…

A: Concentration of acetic acid, HC2H3O2(aq) = 0.00850 M For acetic acid, HC2H3O2(aq), Ka = 1.8×10–5,…

Q: Calculate the pH of a solution obtained by mixing 154.52 mL of 0.28 M CH3COOH with 154.52 mL of 0.28…

A: Note: As per the guidelines, solution of 1st question has been made. For the expert solution of 2nd…

Q: Problem 17.43 - Enhanced - with Feedback A 20.0-mL sample of a 0.200 M HBr solution is titrated with…

A: Part - D 20.2 mL Number of moles of NaOH in 20.2 mL are  :----moles of NaOH = volume (L) ×…

Q: What is the final pH of a solution made by mixing 100 mL of 0.05 M CH3COOH and 100 ml of 0.1 M…

A: A buffer is a solution which resist any change in pH on adding a small amount of acid or base .   it…

Q: 5 i)What is the pH of a mixture made by adding 0.10 mol of acetic acid and 0.050 mol of potassium…

A: Concentration of acetic acid = 0.10 mol  Concentration of potassium acetate=  0.050 mol  Volume of…

Q: Find the pH when 20.00 mL of 0.087 42 M NaOH have been added to 25.00 mL of 0.066 66 M HClO4.

A: We know that, pH and pOH can be expressed as the negative logarithm of H+ and OH- respectively ,…

Q: A solution is prepared at 25 °C that is initially 0.083M in chlorous acid (HCIO,), a weak acid with…

A: Initial concentration of chlorous acid= 0.083 M Ka=1.1×10^-2 Concentration of sodium chlorite =0.065…

Q: mL CSOH added 5.00 10.00 15.00 20.00 25.00 OA HW pKa = 7.46 O B. HD pKa = 5.89 OCHG pKa = 6.85 ÖD.…

A: Molarity of Acid = 0.350 M Volume of Acid = 20 mL Mmol of Acid = M × V      = 0.350 × 20 = 7.0 mmol…

Q: What is the pH if I mix 20.0 mL of 0.100 M HAc, 30.00 of .100 M NaOH, and 20.0 mL of distilled H2O?

A: pH is the measure of acidity or basicity of a solution.  Mathematically, it is the negative…

Q: 8-The following titration curve is the kind of curve expected for the titration of a base (a)…

A: The titration curve is a plot between pH (dependent variable) and the volume of titrant added…

Q: A 0.1276−g sample of a monoprotic acid (molar mass = 1.10 ×102 g/mol) was dissolved in 25.0 mLof…

A: Given, Mass of monoprotic acid = 0.1276 g ( Molar mass = 1.10x 102 g/mol) Volume of water = 25.0 mL.…

Q: You plan to make a buffer solution with sulfurous acid (H₂SO) and it undergoes dissociation reaction…

A: Henderson-Hasselbalch equation is used to prepare a buffer solution of desired pH: Desired pH is…

Q: help please answer in text form with proper workings and explanation for each and every part and…

A: we'll use the given dissociation constant (Ka) for HCN, which is (4.9×10−10). Here are the steps:…

Q: 10-If 25.00 ml of 0.1M NaOH solution is needed to reach the end point of 10 ml HNO₂. Then the…

A: Given, Volume of NaOH = 25.0 ml Conc. of NaOH = 0.1M Volume of HNO3 = 10.0 mlMolecular weight of…

Q: 2-The pH of a 0.02 M solution of an unknown weak acid is 3.7. what is the pK, of this acid? (c) 3.2…

A:

Q: The buffer from Part A is diluted to 1.00 L. To half of it (500. mL), you add 0.0100 mol of hydrogen…

A: Given,  Volume of buffer solution = 500. mL moles of H+ ions = 0.0100 mol

Q: Based on the information from ppt file “add 6M HCl dropwise until the evolution of H2 gas stops and…

A: According to information given in the question, measurement are taken on the basis of evalation of…

Q: What is the pH of a 0.375 L solution made with and 25.00 mL of 5.50 M HBRO (K, = 2.3 x 10 ) 2.775 g…

A:

Q: Calculate the pH of the solution produced when 20.o mL of o.125 M HCI are mixed with 50 mL of each…

A: Given :             Volume of HCl = 20.0 mL            Molarity of HCl = 0.125 M            Volume…

Q: 584.0 mL of a 0.13 M solution of ammonia is mixed with 584.0 mL of a 0.13 M solution of HBr. What is…

A:

Q: G and h

A: Given:

Q: Find the pH when 12.74 mL of 0.087 42 M NaOH have been added to 25.00 mL of 0.066 66 M HClO4.

A: Volume of NaOH  12.74 mL Molarity of NaOH = 0.08742 M Volume of HClO4 = 25.00 mL Molarity of HClO4 =…

Q: Calculate the molar mass of NaF (with solution)

A: The molar mass of the compounds can be defined by the sum of the atomic masses of each atom making…

Q: = 1.01x10-14.) Calculate the pH and the pOH of each of the following solutions at 25°C for which the…

A: So for any acid, base species we can calculate ph and poh easily by calculating H+ -

Q: need

A: Since you have asked multiple question, we will solve the first question for you.If you want any…

Q: The pH of an aqueous solution of 0.237 M ammonium chloride, NH4Cl(aq), is (Assume that Kb (NH3) =…

A: We have to calculate the pH of ammonium chloride solution

Q: A 17.2 mL solution of 0.100 mol L-¹ HF is titrated using 0.150 mol L-1 NaOH. What is the pH of the…

A: Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: Calculate the pH after the addition of the following volumes of 0.2 M NaOH to 30 mL of 0.2 M H₂X…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: Calculate the pH after addition of 10.20 mL of 0.1907 M NaOH to 25.00 mL of 0.1165 M HBr.

A: Given  Volume of NaOH = 10.20 mL Molarity of NaOH = 0.1907 M Volume of HBr  = 25.00 mL Molarity of…

Q: Determine the Ka value [H +]eq Solution 5  4.68 X 10-10 M Directions Take a 30.0 mL sample…

A: The concentration of hydroxyl ion is calculated as follows:

Q: Calculate the pH of a solution formed by mixing 150.0 mL of 0.20 M HClO with 300.0 mL of 0.30 M…

A: Henderson's equations enable the calculation of the pH of buffer solutions prepared by mixing known…

Q: 7) What is the pH of a solution made by mixing 40.00 mL of 0.100 M HCI with 0.100 MK following…

A: Since you have mentioned parts A,B,C,D and E. We are providing you a solution for these parts only.

Q: If one mixes an 0.10M solution of monohydrogen phosphate ion HPO3-2with an equal volume of 0.1M…

A:

Q: What is the pH of a solution prepared by diluting 195.7 mL of 1.55 M HNO3 (Ka>>1) to a total volume…

A: Given :  Initial volume = 195.7 ml  Initial concentration = 1.55 M  Final volume = 8.98 L = 8980 ml…

Q: What

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: Which of the following solutions would be expected to have a pH of 7.00? Weak Ka Kb Base < 10-10…

A: When a salt is formed by reaction of strong acid and strong base , then the salt is neutral salt and…

Q: Calculate the pH of the following: 5) A solution that contains 0.10 M ammonium hydrochloride and…

A: In this solution we have a strong acid HCl which dissociate completely .  And another is a weak acid…

Q: FRQ1: Consider the titration of 25.00 ml of 0.08 M of a weak acid, HA, with 0.125 M NAOH. Calculate…

A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…

Q: Calculate the pH of the solution formed when 34.80 mL of 0.0270 M NaOH is added to 43.10 mL of…

A:

Q: A solution is prepared at 25 °C that is initially 0.49 M in diethylamine ((C,Hs),NH), promide…

A: Given-&gt; Molarity of ((C2H5)2NH)) = 0.49 M Kb = 1.3 × 10-3 ((C2H5)2NH2Br) = 0.36 M

Q: Calculate the pH of the solution formed when 0.00 mL of 0.0440 M NaOH is added to 48.20 mL of 0.0440…

A:

Q: 21) What will be the pH (aq., 25 °C) of 100.0 mL of a solution of 1.00 M C̟H̟NH̟B and 1.50 M C,H,NH,…

A: Firstly Calculate the mmoles of salt, weak base and acid :  salt : C2H5NH3+  , weak base : C2H5NH2…

Q: (b) Calculate the pH at the equivalence point. (You may continue on the next page if you need more…

A:

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.